Question

Write the balanced equation and determine the information requested in each of the following.

1. The number of moles and the mass of water formed by the combustion of 20.0kg of acetylene,C2H2,in an excess of oxygen.

2. Limestone, caco3,dissolves in hydrochloric acid, Hcl, to form calcium chloride, carbon dioxide, and water. How many moles of Hcl are required to dissolve 2.6mol of caco3? How many moles of water are formed?
3.aluminiumoxide reacts with sulphuric acid to form aluminiumsulfate and water

A. how many moles of H2SO4 are required to react with 2.6mol of Al2O3

B. How many moles of Al2(So4)3 are formed?

Answer 1

See explanation.

Step-by-step explanation:

Hello!

In this case, we can proceed as follows:

1. Here, the undergoing chemical reaction is:

`C_2H_2+(5)/(2) O_2\rightarrow 2CO_2+H_2O`

Thus, the moles and mass of water turn out:

`n_(H_2O)=20.0kgC_2H_2*(1000gC_2H_2)/(1kgC_2H_2) *(1molC_2H_2)/(26.04gC_2H_2) *(1molH_2O)/(1molC_2H_2)=768molH_2O\\\\m_(H_2O)=768molH_2O*(18.02gH_2O)/(1molH_2O)=13,840 gH_2O`

2. Here, the undergoing chemical reaction is:

`CaCO_3+2HCl\rightarrow CaCl_2+H_2O+CO_2`

So the required moles of HCl and the yielded of water are:

`n_(CaCO_3)=2.6molHCl*(1molCaCO_3)/(2molHCl)=1.3molCaCO_3\\\\ n_(H_2O)=2.6molHCl*(1molH_2O)/(2molHCl)=1.3molH_2O`

3. Here, the undergoing chemical reaction is:

`Al_2O_3+3H_2SO_4\rightarrow Al_2(SO_4)_3+3H_2O`

Now, we apply each mole ratio obtain:

A.

`n_(H_2SO_4)=2.6molAl_2O_3*(3molH_2SO_4)/(1molAl_2O_3) =7.8molH_2SO_4`

B.

`n_(Al_2(SO_4)_3)=2.6molAl_2O_3*(1molAl_2(SO_4)_3)/(1molAl_2O_3) =2.6molAl_2(SO_4)_3`

Best regards!