Answer:
iron = 15000 kg 95% sulfuric acid = 27646.32 kg
Explanation:
The molar volume to a gas is 22.4 L, which means that a mole of a given gas at 0°C and 1 atm will have a volume os 22.4 L.
1 m3 - 1000 L
4870 m3 - x
x = 4870 * 1000 = 4.87 *10^6 L
1 mole - 22.4 L
y mole - 4.87 * 10^6 L
y = 
= 2,17 *10^5 moles (if 100% of the H2 is used)
as 20% of it is lost, we need to know how much more we need to use.
80% - 2.17 * 10^5 moles
100% - z
z = 
= 2,68*10^5 moles
so we would need 2.68*10^5 moles of iron and sulfuric acid.
1 mole of iron - 56 *10^-3 kg
2.68*10^5 moles - t
t= 2.68*56 *10^2 = 15000 kg
1 mole of sulfuric acid - 98 * 10^-3 kg
2.68*10^5 - u
u = 2.68*98 *10^2 = 26264 kg (if 100%)
95% - 26264 kg
100% - v
v = 
= 27646.32 kg
False, it’s not mechanical energy it’s thermal energy.
No,they just separate away from each other
Answer: the momentum is 6 Kgm/s
Explanation:
M= 5 kg
V= 1.2 m/s
Momentum = MV = 5 x 1.2 = 6 Kgm/s
Answer:
38 L
Explanation:
There is some info missing. I think this is the original question.
<em>Consider the chemical reaction: C(s) + H₂
O(g) ⟶ CO(g) + H₂
(g). How many liters of hydrogen gas is formed from the complete reaction of 15.2 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 360 K.</em>
<em />
Step 1: Write the balanced equation
C(s) + H₂
O(g) ⟶ CO(g) + H₂
(g)
Step 2: Calculate the moles corresponding to 15.2 g of C
The molar mass of C is 12.01 g/mol.
Step 3: Calculate the moles of H₂ produced from 1.27 moles of C
The molar ratio of H₂ to C is 1:1. The moles of H₂ produced are 1/1 × 1.27 mol = 1.27 mol.
Step 4: Calculate the volume of H₂
We will use the ideal gas equation.
