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1. What volume of carbon dioxide is formed, at r.t.p., by burning 100 g of carbon? The equation is:
C(s) + O 2 (g) CO 2 (g).
2. What is the volume of 6.50 mol of nitrogen gas at r.t.p.?
3. What volume would 200 g of SF 6 occupy at room temperature and pressure?
4. Methane reacts with steam to produce carbon monoxide and hydrogen, according the following
equation: CH 4 (g) + H 2 O(g) CO(g) + 3H 2 (g)
What volume of H 2 , at room temperature and pressure, would 20 g of methane produce?
5. Burning propane, C 3 H 8 , forms carbon dioxide and water according to the equation: C 3 H 8 + 5O 2
3CO 2 + 4H 2 O. If 50 dm 3 of CO 2 , at r.t.p., was formed, how many grams of propane was burned?
Two hundred (200) grams of carbon is reacted completely with oxygen to form carbon dioxide. Calculate the volume of CO2 produced. The equation is: C(s) + O2(g) --> CO2(g)
The heat needed to vaporize a certain amount of liquid. A certain substance A has a boiling point of 78℃and substance B has a boiling point of 110℃.Answer the following questions and explain your answer in each case.
1.Which substance has a higher vapor pressure?
2. Which substance has a stronger force of attraction?
3. Which substance has a higher heat of vaporization?
4. Which one will have a higher viscosity?
Choose which term among the following refers to each statements in numbers .
A. Surface tension
B. Viscosity
C. boiling point
D. Heat of vaporization
1. It is responsible for the spherical drops of water and is the reason why some insects can walk on the surface of the water.
2. It is a measure of a liquid’s resistance to flow.
3. The temperature at which the vapor pressure of the liquid is equal to atmospheric pressure.
state the observation that would be made if a similar compound of calcium was used instead of magnesium :Explain
A solution is prepared by mixing 1 g of ethanol (c2h60) with 100 g water to give a final volume of 101 ml. calculate the mole fraction for the solute and solvent and the molality of ethanol in the solution
Calculate the percent by volume of a 120-mL solution that contains 15.0 mL of surcose (C12H22O11)
An oxide of nitrogen contains 63.1% oxygen and has a molar mass of 76.0 g/mol.
a. What is the empirical formula of the compound?
b. What is the molecular formula of the compound?
Calculate the molality of solution containing 240.5g of NH4NO3 (ammonium nitrate) dissolved in 1050.0g of water?
An organic compound is known to be nonvolatile and non electrolyte. A 0.35g sample is dissolved in water and diluted to 150mL. The osmotic pressure is measured as 0.04 atm at 250C. The approximate mass number for this compound is 1400g/mol. From the data provided in this problem and knowing that the density Of the solution is 1.00g/mL
a. Calculate the freezing point of the solutions.
b. Determine if the freezing point change would be a good way to determine the molecular mass of the compound.
c. Would the boiling point change be a better determining factor than the freezing point change?
