Answer:
The answer to the question is
The temperature at which the vapor pressure will be 5.00 times higher than it was at 331 K is 353.0797 K.
Explanation:
To solve the question, we make use of the Clausius-Clapeyron equation as follows
Where P₁ = Initial pressure
P₂ = Final pressure
T₁ = Initial temperature = 331 K
T₂ = Final temperature
dvapH = ΔvapH = Heat of vaporization = 70.83 kJ / mol.
R = Universal gas constant = 8.3145. J K⁻¹ mol⁻¹
We are required to find the temperature when P₂ = 5 × P₁
Therefore we have
= 
or T₂ = 
= 353.0797 K
The vapor pressure be 5.00 times higher than it was at 331 K when the temperature is raised to 353.0797 K.
Answer: b. the volume of water vapour increases
Explanation:
when there's an increase in concentration, the equilibrium favours the forward reaction, more product is produced, froward reaction is faster
Answer:
It only has 7 valence electrons because there are seven electrons in the highest orbital.
Explanation:
Answer:
92.8%
Explanation:
Step 1: Given data
- Mass of lead in the bullet (mPb): 11.6 g
- Mass of tin in the bullet (mSn): 0.5 g
- Mass of antimony in the bullet (mSb): 0.4 g
Step 2: Calculate the total mass of the bullet
The total mass of the bullet is equal to the sum of the masses of the elements that form it.
m = mPb + mSn + mSb = 11.6 g + 0.5 g + 0.4 g = 12.5 g
Step 3: Calculate the mass percentage of Pb in the bullet
We will use the following expression.
%Pb = mPb / m × 100%
%Pb = 11.6 g / 12.5 g × 100% = 92.8%
