I once again am stuck on some problems in this chapter. While there is many more I don't get these six I think would help me with the others I'm stuck on. Would highly appreciate very detailed work shown so I can understand the process and apply to other questions of like nature.

1. Using the the following equation: 2 NAOH + H2SO4 --> 2 H2O + Na2SO4
How many grams of Sodium Sulfate will be formed if you start with 200g of sodium hydroxide and you have an excess of sulfuric acid?

2. Using the following equation: Pb(SO4)2 + 4 LiNO3 --> Pb(NO3)4 + 2 LiSO4
How many grams of lithium nitrate will be needed to make 250g of lithium sulfate, assuming that you have an adequate amount of Lead (IV) sulfate to do the reaction?

3a. In the reaction 2 C8H18 + 25 )2 --> 16 CO2 + 18 H2O, what is the ratio of volumes of O2 to CO2?
3b. If 27.3g of C8H18 are combusted, what mass of water will be produced?
3c. How many molecules of CO2 will be produced?

4. F2 (g) + NH3 (g) --> N2F2 (g) + HF (g)
Identify the limiting reagent for the given combination of reactants. Calculate how many grams of whatever substance will be in excess and how many grams of HF will be made.

5. In a laborator, Qem disolved 11.2 g of sugar in water, and then he poured the solution into a 250-mL volume flask. He added enough water to make the solution exactly 250.00mL. What is the concentration of the solution he prepared?

6. CH4 + 2 O2 --> 2 H2O + CO2
a) If 50.0 L of methane at STP are burned, what volume of carbon dioxide will be produced at STP?
b) If 50.0 L of methane at RTP are burned, what volume of gaseous water at STP is produced?
*If someone could tell me what STP and RTP are that would also be nice*

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Question 4 is finished here.

4. Balance the equation, 4F2 + 2NH3 = N2F2 + ...

Solution Summary

The expert determines how many grams of Sodium Sulfate will be formed if you start with 200g of sodium hydroxide.

1. For the equation, Al + O^2 Al^2O^3 answer the following questions:
a. Balance the above equation.
b. If 10.0 g of Al are used, how many g of oxygen are needed and how many g of product are produced?
?c. If you had 20 moles of Al, how many moles of oxygen would be needed and how many moles of product would be produced?

1) Calculate the density of NO2 gas at 0.970 atm and 33C degree.
2) Calculate the molar mass of a gas if 2.50g occupies 0.885L at 685 torr and 33C degree.
3) Calcium hydride,CaH2 , reacts with water to form hydrogen gas:
CaH2(s)+2H2O(l)>>Ca(OH)2(aq)+2H2(g)
This reaction is sometimes used to inflate life rafts, weath

I am unsure of how to answer this question, 4.68 in Chemistry: The Central Science 11E
a) How many grams of solute are present in 50.0 mL of 0.488 M K2Cr2O7?
b) If 4.00 g of (NH4)2SO4 is dissolved in enough water to form 400 mL of solution, what is the molarity of the solution?
c) How many millilitres of 0.0250 M CuSO4

Need help with the attached 10 chemistry questions.
Please refer to attachment for full questions.
1. Indicate whether each of the following is true or false:
A. C4H10 is an unsaturated compound.
B. A mole of CH4 and a mole of CO2 have the same weight.
C. A mole of CCl4 contains 4 moles of Cl
D. Water is a nonpola

Calculate how many moles of each product would be complete conversion of 1.25 mol of the reactant indicated in boldface, what is the mole ratio used.
C2H3OH (I) + 302(g) 2CO2(g) + 3H2O(g)
N2(g) + O2(g) 2NO(g)
2NaClO2(s) + Cl2(g) 2ClO2(g) + 2NaCl(s)
3H2(g) + N2(g) 2NH3(g)
Calculate the m

A reaction occurs with the following stoichiometry
A + P -> AP
The concentration of A was measured versus time after mixing, the data are the following:
[A](nM) Time (s)
50 0
40 100
30 229
20 411
10

When zinc sulfide is heated in air, zinc oxide and sulfur dioxide forms: 2ZnS(s) + 3O2(g) = 2ZnO(s) + 2SO2(g) How many grams of zinc oxide is formed when 100 grams of zinc sulfide is burned? Assume that the zinc sulfide is the limiting reactant.
The answer is one of the following:
a. 8.5 grams ZnO
b. 23.5 grams ZnO
c. 4

Magnesium can be used as a "getter" in evacuated enclosures, to react with the last traces of oxygen. (The magnesium is usually heated by passing an electric current through a wire or ribbon of the metal.)
If an enclosure of 0.384 L has a partial pressure of O2 of 3.6×10−6 torr at 28 C degrees, what mass of magnesium