选择题专题训练9—12

1．下列排列顺序正确的是

①热稳定性：H2O＞HF＞H2S ②原子半径：Na＞Mg＞O

③酸性：H3PO4＞H2SO4＞HClO4④结合质子能力：OH-＞HCO3-＞CH3COO-

A．①③B．②④C．①④D．②③

2．某液体分散系所表现出来的下列性质既可能是胶体所具有，也可能是溶液所具有的是A．光线透过时，从侧面可观察到一条光亮的通路

B．加入稀H2SO4，立即产生沉淀

C．分散质微粒直径小于1nm

D．装入半透膜袋中并将其浸入盛水的烧杯中一段时间，结果袋内外部均有分散质微粒

3．已知X、Y、Z三种元素组成的化合物是离子晶体，其晶胞如下图所示，则下

面表示该化合物的化学式正确的是

A．ZXY3 B．ZX2Y6

C．ZX4Y8 D．ZX8Y12

4．将锌片和铜片用导线连接置于同一稀硫酸溶液中，下列叙述正确的是

A．正极附近SO42－的浓度逐渐增大B．负极附近SO42－的浓度逐渐减小

C．负极附近SO42－的浓度逐渐增大D．正极附近SO42－的浓度基本不变

5．下列相关说法正确的是

A．Zn(s)+CuSO4(aq)=Cu(s)+ZnSO4(aq) △H=－216kJ/mol 反应物总能量生＞生成物总能量

B．CaCO3(s) =CaO(s)+CO2(g) △H=＋178.5kJ/mol 反应物总能量生＞生成物总能量

C．101kPa时2H2(g)+ O2(g)=2H2O (l) △H=－571.6kJ/mol H2的燃烧热是571.6kJ/mol

D．H＋((aq)+HO－(aq)= H2O (l) △H=－57.3kJ/mol含1molNaOH的氢氧化钠溶液与含0.5molH2SO4的浓硫酸混合后放出57.3kJ 的热量

6．测定硫酸铜晶体中含结晶水的实验，造成结果偏高的原因是下列四项中的（）

①坩埚用水洗后没有烘干②加热时有少量晶体溅出

③把加热得到的白色粉末放在空气中冷却、称量④加热完了粉末中有少量的黑色固体

A．①②③B．①②C．②③D．①②④

7．将两个铂电极插入氢氧化钾溶液中，向两极分别通入甲烷和氧气，即构成甲烷燃料电池，已知通入甲烷的一极，其电极反应为：CH4– 8e－+10OH－= CO32－+ 7H2O；通入氧气的另一极，其电极反应式是2O2 + 4H2O + 8e－= 8OH－，下列叙述正确的是（）

A．通入甲烷的电极为正极B．正极发生氧化反应

C．该电池使用一段时间后应补充氢氧化钾D．燃料电池工作时，溶液中的阴离子向正极移动8．下列说法正确的是：( )

A．1mol铜与足量硫充分反应生成转移电子数目为1 N A

B．常温常压下，31g白磷分子中的共价键数为6N A

C．可以利用下面反应设计原电池H2SO4(aq)+BaCl2(aq)=2HCl(aq)+BaSO4(s)；ΔH<0

D．H2O分子受热不发生分解，是由于水分子之间存在氢键

1．下列说法正确的是（）

A．海水是一个巨大的宝藏，对人类生活产生重要影响的元素，如：氯、溴、碘、钠、钾、铁等元素主要来自于海水B．利用风能发电、采取节能技术、使用太阳能热水器、用无氟制冷剂均有利于降低大气中的二氧化碳C．氢氧燃料电池要进入广泛的实际应用，高容量储氢材料的研制是需解决的关键技术问题之一D．生活垃圾焚烧发电不会产生有毒有害物质

2．下列情况下，离子一定可以大量共存的是（）

A．常温下，pH=7的溶液：Na＋、SO42－、Fe3＋、Cl－

B．常温下，水电离的c(H＋)=10－13 mol/L的溶液：K＋、Cl－、Ca2＋、ClO－

C．NH4＋大量存在的溶液：Na＋、NO3－、K＋、CO32－

D．能使甲基橙变红的溶液：Na＋、NH4＋、Fe2＋、NO－3

3．下列说法不正确

．．．的是

A．分别用H2O2、KMnO4分解制O2，当制得等质量的O2时，转移电子数之比为1∶2

B．第三周期主族元素的最高正化合价等于它所处的主族的族序数

C．在共价化合物形成的晶体中除了是原子晶体，其余全部是分子晶体

D．HI的相对原子质量大于HF，则HI的沸点高于HF

4．短周期元素W、X、Y、Z的原子序数依次增大，W与Y、X与Z位于同一主族，W与X可形成共价化合物WX2，Y原子的内层电子总数是其最外层电子数的2.5倍。下列叙述中正确的是（）A．1 mol YX2中含有2 mol的Y—X共价键B．原子半径大小顺序为X < W < Y < Z

C．ZX2是以极性键结合成的极性分子

D．由WX2可知所有的分子晶体中都存在范德华力，分子内都存在共价键

5．LiFePO4新型锂离子动力电池以其独特的优势成为奥运会绿色能源的新宠，已知该电池放电时的电极反应式为：正极FePO4 + Li＋+e－＝LiFePO4，负极Li－e－＝Li＋。下列说法正确的是（）

A．充电时，电池的总反应为FePO4 + Li ＝LiFePO4

B．放电时，在正极上是Li＋得电子被还原，每转移1 mol电子，则生成1 mol LiFePO4

C．放电时，电池内部Li＋向负极移动，电子只能通过外电路由负极到正极

D．充电时，动力电池上标注“+”的电极应与外接电源的正极相连

6．已知还原性：Fe2+＞Br－＞Cl－，在FeCl2、FeBr2的混合溶液中，Cl－、Br－两种离子的物质的量之比为1∶2，向该溶液中通入一定量的氯气，使溶液中Cl－与Br－的个数比为8∶1，则通入氯气的物质的量与原溶液中Fe2＋的物质的量之比为（）

A．1∶1 B．2∶1 C．4∶3 D．2∶3

7．室温下，向1 L 0.01 mol/L的氯水中加入0.8 g NaOH固体，充分反应后，仍维持室温不变(忽略体积

改变)。下列有关反应后溶液中离子浓度的说法不正确

．．．的是

A．0.5c(Na＋) + c(H＋)＝c(OH－) + c(ClO－) B．c(Na＋)＝c(HClO) + c(ClO－)

C．c(Na＋)＞c(Cl－)＞c(ClO－)＞c(OH－)＞c(H＋) D．c(OH－) + c(ClO－)―c(H＋)＝0.01 mol/L 8．常温下，向100 mL某稀硫酸和稀硝酸的混合溶液中加入铜粉，最多能

溶解19.2 g（已知硝酸只被还原为NO气体）。若再取等体积的该混酸溶

液向其中逐渐加入铁粉，产生气体的量随铁粉质量增加的变化如右图所

示。下列分析或结果错误的是

A．取10 mL原混合酸溶液加入水稀释至1 L后，其pH = 2

B．100 mL混合酸中NO3－物质的量为0.2 mol

C．原混合酸中，H2SO4物质的量浓度为4 mol·L－1

D．OA段产生的是NO，AB段的反应为Fe+ 2Fe3＋= 3Fe2＋，BC段产生氢气

1. 下列反应能实现的是

A ．H 2SO 3 + X 2 + H 2O = 2HX + H 2SO 4 (X 2表示Cl 2、Br 2、I 2)

B ．热的浓H 2SO 4能与A 反应生成AO 2 (A 表示

C 、S 、P)

C ．M + S MS (M 表示Zn 、Fe 、Cu)

D ．M + 2H 2SO 4(浓) MSO 4 + SO 2↑+ 2H 2O (M 表示Zn 、Fe 、Cu)

2. 下列实验操作中，错误的是（）

A ．金属钠与水反应时，需要用滤纸将金属钠表面的煤油吸干

B ．一定物质的量浓度的测定实验中，容量瓶需要用待装液润洗

C ．Ba(OH)2·8H 2O 和NH 4Cl 反应时，应在玻璃片上事先滴少量水

D ．中和热测定实验中，应用环型玻璃搅拌棒轻轻搅动混合液

3. X 、Y 、Z 、W 是原子序数依次增大的短周期元素，且互不同族，其中只有两种为金属；X 原子的最外层电子数与次外层电子数相等；X 与W 、Y 与Z 这两对原子的最外层电子数之和均为9。单质Y 和W 都可与NaOH 溶液反应。下列说法不正确．．．

的是

A ．原子半径：Y>Z>W

B ．XW 2熔点为107℃，沸点为12.5℃，说明固态XW 2为分子晶体

C ．YW 3水溶液蒸干并灼烧可得YW 3固体

D ．ZW 2分子结构见右图，说明ZW 2是极性分子

4. 常温常压下，在带有相同质量活塞的容积相等的甲、乙两容器里，分别充有二氧化氮和空气，现

分别进行下列两个实验：（N 2O

42NO 2 △H ＞0）

（a ）将两容器置于沸水中加热（b ）在活塞上都加2 kg 的砝码

在以上两种情况下，甲和乙容器的体积大小的比较，正确的是

A ．（a ）甲＞乙，（b ）甲＞乙

B ．（a ）甲＞乙，（b ）甲＝乙

C ．（a ）甲＜乙，（b ）甲＞乙

D ．（a ）甲＞乙，（b ）甲＜乙 5. 在体积不变的密闭容器中进行可逆反应：

3A(g) + B(?)

C(g) + 2D(?)；△H ＜0，达到平衡后升高温度，气体的平均相对分子质量减小，则下列说法错误．．的是

A ．

B 、D 可能都是气体 B ．可能B 为非气体，D 为气体

C ．容器内气体密度一定减小

D ．等倍数增大各种反应物和生成物的物质的量，达到新平衡时，A 的百分含量的可能会不变

6. 短周期的A 、B 两种元素，A 原子半径小于B 原子半径，两种元素可形成A 是正价的AB 2型化合物。下列关于两元素的叙述正确的是

①A 、B 可能属于同一周期； ②A 是B 的前一周期元素；

③A 只能是金属元素； ④A 可能是第二周期IIA 族或IV A 族元素

A ．①③

B ．②③

C ．②④

D ．②③④

7. 在容积为V L 的密闭容器中发生2NO 2(g)2NO(g) + O 2(g)的可逆反应。开

始时，只充入NO 2，反应过程中NO 2物质的量随时间变化的情况如右图所示（曲

线A 和B 表示的是该反应在某不同条件下的反应情况）。下列有关叙述正确的是

A ．与曲线A 相比较，曲线

B 的反应条件可能是增大了压强

B ．与曲线A 相比较，曲线B 的反应条件可能是升高了温度

C ．在曲线B 条件下达平衡时，O 2的平均反应速率为0.1/(Vt 1)mol ·L －1·min

－1

D ．其它条件不变，升高温度，该平衡向逆反应方向移动

甲乙

1.下列化工生产过程中不涉及

．．．氧化还原反应的是

A．氯碱工业B．硫酸工业

C．玻璃工业D．合成氨工业

2.下列各组离子在水溶液中能大量共存，在酸性条件下能发生氧化还原反应的是

A．Mg2+、Al3+、SO42—、C1—B．K+、Na+、SO32—、NO3—

C．Na+、Fe3+、SCN—、SO42—D．NH4+、Na+、C1—、CO32—

3.设N A表示阿伏加德罗常数，下列有关说法正确的是

A．25℃时，1 L pH=13的NaOH溶液中约含有0．1 N A个氢氧根离子

B．53．5g NH4Cl中含有H—Cl键的个数为4N A

C．1 mol羟基（-OH）所含的电子数约为10N A

D．在标准状况下，2．24L的己烷中含有C—H键的数目约为0．6N A

4.相关实验不能

．．表达预期目的的是

选择题专题训练(17) .doc

选择题专题训练（17）姓名班级学号 1．化学知识广泛应用于生产、生活中，下列相关说法不．正确．．的是（） A ．食用松花蛋时蘸些食醋可以去除氨的气味 B ．棉花和木材的主要成分都是纤维素，蚕丝的主要成分是蛋白质 C ．只用淀粉溶液即可检验食盐是否为加碘盐 D ．液氯罐泄漏时，可将其移入水塘中，并向水塘中加入生石灰 2．已知在101kPa 时：CH 4(g)＋2O 2(g)＝CO 2(g)＋2H 2O(g)；△H＝-820kJ/mol 。下列说法中正确的是（） A ．反应过程中能量关系可用右图表示 B ．CH 4的燃烧热是820kJ C ．11.2LCH 4完全燃烧放出热量410kJ D ．若将此反应设计成原电池，甲烷在正极被氧化3．用N A 表示阿伏加德罗常数，下列说法不．正确．．的是（） A ．0.2mol 过氧化氢完全分解生成0.1molO 2时转移的电子数目为0.2N A B ．300mL2mol/L 蔗糖溶液中所含分子数为0.6N A C ．在常温常压下，17g 硫化氢气体所含质子数目为9N A D ．在标准状况下，2.24L 二氧化硫与氧气混合气体中所含氧原子数为0.2N A 4．用下列实验装置完成对应的实验（部分仪器已省略），操作正确并能达到实验目的的是（） A ．干燥Cl 2 B ．检验K 2CO 3中的K + C ．石油的蒸馏 D ．吸收NH 3 5．下列有关化学用语的叙述正确的是（） A ．硫酸铝水解的化学方程式是：Al 2(SO 4)3＋3H 2O 2Al(OH)3＋3H 2SO 4 B ．铜跟浓硝酸反应的离子方程式是：Cu ＋4NHO 3(浓)＝Cu 2+ ＋2NO 3- ＋2NO 2↑＋2H 2O C ．钢铁发生吸氧腐蚀时，负极发生的电极反应为：2H 2O ＋O 2＋4e -→4OH - D ．氢氧化亚铁在空气中久置变成红褐色的化学方程式为： Cl 2 浓H 2SO 4 NH 3 稀H 2SO 4 C 6H 6 生成物能量总和反应过程中放出的能量反应物能量总和能量反应进程

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