Question

For the reaction below, calculate how many moles of the product form when 0.026 mol of O2 completely reacts. Assume that there is more than enough of the other reactant.

2Ca(s)+O2(g)→2CaO(s)

Express your answer using two significant figures.

Answer #1

In a balanced chemical reaction the numbers signify the mole numbers used in the reaction.

So from the above reaction we can easily say that from one mole oxygen two moles of CaO is produced. That means if we start from 1 mole of oxygen and after it fully reacts we will end up with 2 moles of product.

Here we have started this reaction with 0.026 moles of O2. Thus after complete reaction we will have 2*0.026=0.052 moles of product.

To complete the reaction the other reactant which is Ca here must be sufficient. So the condition of excess Ca is given.

For the reaction, calculate how many moles of the product form
when 0.046 mol of O2 completely reacts.
Assume that there is more than enough of the other reactant.
2Ca(s)+O2(g)→2CaO(s)
For the reaction, calculate how many moles of the product form
when 0.018 mol of O2 completely reacts.
Assume that there is more than enough of the other reactant.
4Fe(s)+3O2(g)→2Fe2O3(s)
For the reaction, calculate how many moles of the product form
when 0.044 mol of K completely reacts.
Assume that...

(Part A) For the reaction, calculate how many grams of the
product form when 16.4 g of O2 completely reacts.
Assume that there is more than enough of the other reactant.
4Cr(s)+3O2(g)→2Cr2O3(s)
(Part B) For the reaction, calculate how many grams of the
product form when 16.4 g of Sr completely reacts.
Assume that there is more than enough of the other reactant.
2Sr(s)+O2(g)→2SrO(s)

For the reaction, calculate how many grams of the product form
when 24.4 g of O2 completely reacts.
Assume that there is more than enough of the other reactant.
4Cr(s)+3O2(g)→2Cr2O3(s)

(Part A) For the reaction, calculate how many grams of the
product form when 16.4 g of Ca completely reacts.
Assume that there is more than enough of the other reactant.
Ca(s)+Cl2(g)→CaCl2(s)
(Part B) For the reaction, calculate how many grams of the
product form when 16.4 g of Br2 completely reacts.
Assume that there is more than enough of the other reactant.
2K(s)+Br2(l)→2KBr(s)

For the reaction shown, calculate how many moles of NO2 form
when each amount of reactant completely reacts.
2N2O5(g)→4NO2(g)+O2(g)
Part B
5.3 molN2O5 (Express your answer using two significant
figures.)
Part C
4.76×103molN2O5 (Express your answer using three significant
figures.)
Part D
1.015×10−3molN2O5 (Express your answer using four
significant figures.)

For the reaction shown, calculate how many moles of NO2 form
when each amount of reactant completely reacts.
2N2O5(g)→4NO2(g)+O2(g)
a. 6.4 mol N2O5
b. 10.0 g N2O5
c. 1.55 kg N2O5

For the reaction shown, calculate how many grams of each product
form when the following amounts of reactant completely react to
form products. Assume that there is more than enough of the other
reactant. 2Al(s)+Fe2O3(s)→Al2O3(s)+2Fe(l)
A.) 4.0 gFe2O3

1.Calculate how many moles of NH3 form when each quantity of
reactant completely reacts according to the equation:
3N2H4(l)→4NH3(g)+N2(g)
4.10 mol N2H4
65.8 g N2H4
Hydrobromic acid dissolves solid iron according to the following
reaction:
2.Fe(s)+2HBr(aq)→FeBr2(aq)+H2(g)
What mass of HBr (in g) would you need to dissolve a 3.2 −g pure
iron bar on a padlock?
Express your answer using two significant figures.
What mass of H2 would be produced by the complete reaction of
the iron bar?
Express your...

CaO(s)−−−−−−+CO2(g)→CaCO3(s)
Express your answer using two significant figures.
For each reaction, calculate the mass (in grams) of the product
formed when 2.9 g of the underlined reactant completely reacts.
Assume that there is more than enough of the other reactant.
Ba(s)−−−−−+Cl2(g)→BaCl2(s)
Express your answer using two significant figures.
2Mg(s)−−−−−+O2(g)→2MgO(s)
Express your answer using two significant figures.
4Al(s)−−−−−+3O2(g)→2Al2O3(s)
Express your answer using two significant figures.

For each of the reactions, calculate the mass (in grams) of the
product formed when 15.82 g of the underlined reactant completely
reacts. Assume that there is more than enough of the other
reactant.
Express your answer using four significant figures.
1) 2K(s)+Cl2(g)−−−−−→2KCl(s)
2) 2K(s)+Br2(l)−−−−−→2KBr(s)
3) 4Cr(s)+3O2(g)−−−−−→2Cr2O3(s)

ADVERTISEMENT

Get Answers For Free

Most questions answered within 1 hours.

ADVERTISEMENT

asked 12 minutes ago

asked 15 minutes ago

asked 33 minutes ago

asked 57 minutes ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 1 hour ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago

asked 2 hours ago