The first part of two is heat, not temperature, once that is cleared up: starting from 3: temperature, concentration, collisions, catalytic converter, surface area
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Hello!</h2>
The answer is: The new pressure of the gas is 3.6 atm.
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Why?</h2>
From the statement we know that the gas is kept at a constant temperature of 0°C, so, if the gas keeps a constant temperature we can use the Boyle's Law to solve this problem.
The Boyle's Law states that:
Where,
P is the pressure of the gas.
V is the volume of the gas.
So, the given information is:
Now, substituting it into the Boyle's Law equation to calculate the new pressure, we have:
So, the new pressure is 3.6 atm.
Have a nice day!
Answer:
40.5% is abundance of X-122
Explanation:
we know there are two naturally occurring isotopes of X, X-120 and X-122.
First of all we will set the fraction for both isotopes
X for the isotopes having mass 122
1-x for isotopes having mass 12
0
The average atomic mass of X is 120.81 amu
we will use the following equation,
122x + 120 (1-x) = 120.81
122x + 120 - 120x = 120.81
122x- 120x = 120.81 -120
2x = 0.81
x= 0.81/2
x= 0.405
0.405 × 100 = 40.5%
40.5% is abundance of X-122 because we solve the fraction x.
now we will calculate the abundance of X-120.
(1-x)
1 - 0.405 = 0.595
0.595 × 100 = 59.5 %
59.5 % for X-120.
Answer:
Complete ionic equation:
2H²⁺(aq) + SO₄²⁻(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + Ca²⁺(aq) + SO₄²⁻(aq)
Net ionic equation:
2H²⁺(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + Ca²⁺(aq)
Explanation:
Chemical equation:
H₂SO₄(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + CaSO₄(aq)
Balanced chemical equation:
H₂SO₄(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + CaSO₄(aq)
Complete ionic equation:
2H²⁺(aq) + SO₄²⁻(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + Ca²⁺(aq) + SO₄²⁻(aq)
Net ionic equation:
2H²⁺(aq) + CaCO₃(s) → H₂O(l) + CO₂(g) + Ca²⁺(aq)
