The given question is incomplete, the complete question is:
A reaction between liquid reactants takes place at 10.0 °c in a sealed, evacuated vessel with a measured volume of 35.0 L. Measurements show that the reaction produced 28. g of dinitrogen difluoride gas. Calculate the pressure of dinitrogen difluoride gas in the reaction vessel after the reaction. You may ignore the volume of the liquid reactants. Round your answer to 2 significant digits. pressure:atm
Answer:
The correct answer is 0.28 atm.
Explanation:
The temperature mentioned in the given reaction is 10 degree C, which after conversion becomes 283 Kelvin (273+10 = 283K).
The volume mentioned in the reaction is 35 Liters.
The reaction produced 28 grams of dinitrogen difluoride gas (N2F2). The n or the no of moles of the gas can be determined with the help of the formula:
moles of N2F2 = mass/molar mass
= 28/66 (molar mass of N2F2 is 66 g/mol)
= 0.424
The pressure of the gas can be determined by using the equation of the ideal gas law, that is, PV = nRT
P * 35 = 0.424 * 0.0821 * 283
P = 0.28 atm
<span>c. The molecules are closer together as a gas than they do as a liquid.</span>
Homogeneous because it is unable to be distinguished of the components Water and Salt
Answer:
The half-reaction for the oxidation of the manganese in 
to 
.:
Explanation:
Let us say the medium in which reaction is taking place is an acidic medium. And balancing in an acidic mediums done as;
Step 1: Balance all the atom beside oxygen and hydrogen atom;
Manganese and carbon are balanced.
Step 2: Balance oxygen atom adding water on the required side:
Step 3: Now balance hydrogen atom by adding hydrogen ion on the required side:
Answer:4.48483134×10 to the power of 19 m to the power of 2/s
Explanation:
You should work it out some and see
