Answer:
9.0 L.
Explanation:
- To solve this problem, we should use the general gas law of ideal gas:
PV = nRT.
where,
P is the pressure of the gas in (atm).
V is the volume of the gas in (L).
n is the no. of moles of the gas (mol).
R is the general constant for gases (R = 0.082 L.atm/mol.K).
T is the temperature of the gas in (K).
- Since the P, T and R are constants, the variables are V and n.
<em>∴ V₁n₂ = V₂n₁.</em>
V₁ = 6.0 L & n₁ = 0.50 mol.
V₂ = ??? L & n₂ = 0.75 mol.
∴ V₂ = (V₁n₂) / (n₁) = (6.0 L)(0.75 mol) / (0.50 mol) = 9.0 L.
Answer:
80cm3 of water, and 60cm3 carbon IV oxide is formed while 20cm3 of oxygen is left unreacted.
Explanation:
From Gay-Lussac's law, there are five volumes of oxygen, 1 volume if propane, 4 volumes of water and three volumes of CO2. Applying this shows the reacting volumes as we have in the image attached, hence the volumes left after reaction.
Some of the particles undergo a phase change and become a gas due to burning. An example would be CO2, which is lost in the air around/escapes into the atmosphere. Hope that helps!
I believe the answer is D. An ion always has a positive or a negative charge. An Ion is an atom with net electric charge due to the loss or gain of one or more electrons. An isotope is each of two or more forms of the same element that contain equal numbers of protons but different numbers of neutrons in their neutron, thus they differ in relative atomic mass but not in chemical properties.
