Answer:
i think its CaCO3 + 2HCl → CaCl2 + H2O + CO2
Explanation:
Answer:
The percentage yield is 78.2g
Explanation:
Given, mass of propane = 42.8 g , sufficient O2 percent yield = 61.0 % yield.
Reaction - C3H8(g)+5O2(g)------> 3CO2(g)+4H2O(g)
First we need to calculate the moles of propane
Moles of propane = 
g.mol-1
= 0.971 moles
So, moles of CO2 from the moles of propane
1 mole of C3H8(g) = 3 moles of CO2(g)
So, 0.971 moles of C3H8(g) = ?
= 2.913 moles of CO2
So theoretical yield = 2.913 moles 
44.0 g/mol
= 128.2 g
So, the actual mass of CO2 = percent yield theoretical yield / 100 %
= 61.0 % 128.2 g / 100 %
= 78.2 g
the mass of CO2 that can be produced if the reaction of 42.8 g of propane and sufficient oxygen has a 61.0 % yield is 78.2 g
Answer:
A) Has properties of both metals and nonmetals - Barium.
B) Nonreactive gas - Neon.
C) Great conductor of heat and electricity - Boron.
D) Malleable and highly reactive - Potassium.
Explanation:
hope it helps .
Answer:
The average kinetic energy of the gas particles is greater in container B because it has a higher temperature.
Explanation:
<em>The correct option would be that the average kinetic energy of the gas particles is greater in container B because it has a higher temperature.</em>
<u>According to the kinetic theory of matter, the temperate of a substance is a measure of the average kinetic energy of the molecules of substance. In other words, the higher the temperature of a substance, the higher the average kinetic energy of the molecules of the substance.</u>
In the illustration, the gas in container B showed a higher temperature than that of container A as indicated on the thermometer, it thus means that the average kinetic energy of the molecules of gas B is higher than those of gas A.
