Chemistry Answers

What type of reagent is required to convert No2 to N2

4. If you had 36.2 grams of aluminum metal reaction with 45.0 grams of copper (II) hydroxide,

which is the limiting and which is the excess reactant?

5. How many grams of copper metal would be produced?

6.How much of the excess reactant is left when the reaction stops?

3. Too make exactly 100. grams of ferric sulfate how many grams of sulfuric acid would be

needed?

4. If you had 36.2 grams of aluminum metal reaction with 45.0 grams of copper (II) hydroxide,

which is the limiting and which is the excess reactant?

1. If you had 6.50 moles of ferric hydroxide how many grams of ferric sulfate will be produced?

2. If 25.7 grams of water was produced what is the amount of sulfuric acid needed to produce the

water?

what are the reactions for

Mg+Pb(NO)3=Mg(NO3)2

C2H6=CO2 +H2O

The density of air at 20°C and 1.00 atm is 1.205 g/L. If this air were compressed at the 

same temperature to equal the pressure at 40.0 m below sea level, what would be its 

density? Assume the barometric pressure is constant at 1.00 atm. The density of seawater 

is 1.025 g/cm3

.

 â€˜Undecane’ is a straight chain alkane containing how many carbon atoms?

What is the purpose for a company to determine percent yield of a product and not just the theoretical yield?

• The percent yield enables the calculation for the exact amount of product that can be expected, which may help determine profit, an accurate amount of reactant to use, and the efficiency of the system.
• The percent yield enables the calculation of the maximum amount of error that can be expected, which may help determine loss of profit, minimal amount of reactant to use, and the inefficiency of the system.
• The percent yield enables the calculation of the maximum amount of product that can be expected, which may help determine loss of profit, minimal amount of reactant to use, and the inefficiency of the system.

select which of the options

How many mol of NO are produced from a reaction if its mass is 2.05 g?

Periodic Table Reference Sheet

• 1.46 × 10² mol NO
• 6.83 × 10^–2 mol NO
• 1.28 × 10^–1 mol NO
• 6.15 × 10¹ mol NO

it's NOT: 6.15 × 10¹ mol NO or 1.46 × 10² mol NO

If Ag2O decomposes, what is the balanced equation that shows the products formed?

• 2Ag2O(s) → 4Ag(s) + O2(g)
• Ag2O(s) → Ag2(s) + O(g)
• 2Ag2O(s) → 4Ag(s) + 2O(g)
• Ag2O(s) → 2Ag(s) + O(g)

it's NOT: Ag2O(s) → Ag2(s) + O(g)