Question

** Stoichiometry, Limiting Reactants and Percent Yield**

Answer 1

I have a big Chapter test tomorrow. Will somebody pleaseee check my study guide for errors??? PLEASE

Answer 2

@Panda.exe

Answer 3

ok

Answer 4

#9 has the equation: 2K + CL2 --> 2KCL

Answer 5

The question is: How many moles of KCL are produced from 2.50 moles K?

Answer 6

I got 2.5 moles KCL....is that right?

Answer 7

yes it is

Answer 8

great haha thanks..i have a few more..if thats okay?

Answer 9

Yes idc

Answer 10

jesse u there

Answer 11

Equation: 3 NO2 + H20 --> 2HNO3 + NO

Question: What mass of water is required to react with 15.5 L of Nitrogen Dioxide?

My Answer: 12.5 Grams H2O

Answer 12

correct

Answer 13

Another question to the same equation: What volume of Nitrogen Monoxide would be produced from 100.0 g of water?

My answer: 124 Liters of NO

Answer 14

no Its 373.4

Answer 15

\[100H2O\div1\times1molsNO \times22.4LNO \div1molsNO\]

Answer 16

Thats what i did...i wonder what i did wrong?

Answer 17

nvm i was rong its right xD

Answer 18

wrong

Answer 19

ok jesse next

Answer 20

The third question is:
IF 42.0 L of NO is produced, what volume of NO2 reacted?

My answer: 126 L NO2

Answer 21

lol 420 and yes

Answer 22

lmao okay

Answer 23

umm now this question is Limiting the reactants

Answer 24

idk how to do the rest of them srry

Answer 25

Equation: Zn + Cu(NO3)2 --> Cu + Zn(NO3)2
Question: iF 100 g of zinc metal and 100 g of copper(II) nitrate react, how many grams of copper metal will be produced according to the equation? What is the limiting Reactant?

Answer 26

I got 98 g Cu from 100 grams Zn and 34 g Cu from 100 grams Cu(NO3)2. The limiting reactant is Cu(NO3)2........correct?