The choices are:
<span>A. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 0</span>°<span>C.
B. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 298 K.
C. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 273</span>°<span> C.
D. The first gas sample has a temperature of 273 K, and the second gas sample has a temperature of 100</span>°<span> C.
The correct answer is A because the two gases will have the same temperature and 273 K = 0</span>°C
Answer:
Faster
number
reactants
increases
Explanation:
The rate of reaction refers to how fast or slow a reaction occurs. The rate of reaction is dependent on factors such as surface area, concentration, temperature, nature of reactants, catalyst etc.
The concentration refers to the amount of reactants present. When the acid is made more concentrated, its amount is increased. This increases the number of collisions between the acid particles and the marble chips ultimately leading to increase in the rate of reaction according to Arrhenius theory.
Answer:
Explanation:
1. Gather the information
We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.
Mᵣ: 16.04 32.00 44.01
CH₄ + 2O₂ ⟶ CO₂ + 2H₂O
m/g: 60
1. Moles of CO₂
2. Mass of CH₄
(a) Moles of CH₄
(b) Mass of CH₄
3. Mass of O₂ required
(a) Moles of O₂
(b) Mass of O₂
Your answer would be c
hope this helps