A student carried heated a 25.00 g piece of aluminum to a temperature of 100°C, and placed it in 100.00 g of water, initially at
1 answer:
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Answer:
0.264 moles of carbon dioxide are produced.
Explanation:
<u>Limiting reagent</u> : The reactant that is consumed in a reaction is called the limiting reagent.
Molar mass = mass of substance in grams present in 1 mole of the compound.
before solving this question,
It is needed to know , the molar mass of cr2(co3)3 and CO2
Molar mass of cr2(co3)3 = 2(mass of Cr) + 3(massof C) + 9(mass of O)
= 2(52) + 3(12) + 9(16)
= 104 + 36 + 144
= 284 g
This means 1 mole of cr2(co3)3 = 284 g............(1)
Molar mass of CO2 = mass of C + 2(mass of O)
= 12 + 2(16)
= 12 + 32
= 44 g
This means 1 mole of CO2 contain 44 g of it.
So, 3 mole of CO2 contain = 44x3 g
3 mole of CO2 contain = 132 g.............(2)
The balance equation for the reaction is :
HNO3 = excess reagent , it can't be used in for predicting the moles of CO2
= Limiting reagent = It will tell the amount of CO2 that will be produced
In the balanced equation ,
1 mole of cr2(co3)3 is giving = 3 mole of CO2
Use equation (1) and (2)
284 g of cr2(co3)3 is giving = 132 g of CO2
1 gram of cr2(co3)3 is giving =
g of CO2
25 g of cr2(co3)3 will give =
g of CO2
= 11.62 gram CO2
now , moles of CO2 can be calculated using ,
(molar mass of co2 = 44 g)
moles of CO2 = 0.264
Answer : The diatomic gas is nitrogen gas, N₂.
Explanation :
First we have to calculate the moles of gas.
Using ideal gas equation:
where,
P = Pressure of gas = 1.00 atm
V = Volume of gas = 4.4 L
n = number of moles of gas = ?
R = Gas constant =
T = Temperature of gas =
Putting values in above equation, we get:
Now we have to calculate the molar mass of gas.
As we are given that the gas is diatomic X₂.
As, 2 atoms of gas X has mass = 28.07 g/mol
So, 1 atom of gas will have mass =
From this we conclude that the nitrogen atom has mass of 14.04 g/mol.
Thus, the diatomic gas is nitrogen gas, N₂.