General Chemistry Answers

1. You have ice at 263K (-10.0oC) and 1.0 atm. What could you do to make the ice sublime? A sample of dry ice (solid CO2) is cooled to 173K (-100.0oC), and is set on a table at room temperature (298 K; 25 oC). At what temperature is the rate of sublimation and deposition the same (assume that pressure is held constant at 1 atm)?

What Concentration Of CH4 Is Used Up After 10 Minutes

2 C₈H₁₈(l) + 25 O₂(g)  16 CO₂(g) + 18 H₂O(l)

Calculate the ΔH° for the combustion of octane shown above. The ΔH°_f of octane is -652.7 kJ/mol. Use the thermodynamic values in these Reference Tables. Round your answer to the number of decimal places allowed by the data.

 answer in kJ

Aluminum has a specific heat of 0.900 J/g·°C. How much energy is required to raise the temperature of 140. g of aluminum from 10.0°C to 232.0°C? Answer in kJ

Calculate the final temperature after 262 J of heat is added to 56.2 g of magnesium at 14.0°C.

---------------°C

What happens if I mix glycerine and hand sanitiser and use in fumigation process(Heat) . Does the smoke produced, still have effect of killing the virus and sanitization?

What is the general trend in the size of atomic radii as the atomic number increases within a group?

 Here is a balanced equation. Use it to answer the questions below.

2Pb(NO3)2     🠖     2PbO     +     4NO2    +     O2

(i). How many moles of nitrogen dioxide would you be able to get from 2 moles of lead(II) nitrate?

(ii). How many moles of oxygen would you be able to get from 1 mole of lead (II) nitrate? 

(iii). What mass of PbO could be obtained from 200g of Pb(NO3)2?

(iv). If 130.0g of PbO are actually obtained when the experiment is done in the laboratory, what is the percentage yield?

7. A sample of sodium hydroxide of mass 1.600g is added to a solution containing 1.472g of H2SO4.

2NaOH     +     H2SO4     →     Na2SO4     +     2H2O

a). Identify the limiting reactant.

b). Calculate the mass of sodium sulfate formed in the solution.

c). Calculate the mass of the unused reactant remaining in the solution.

When hydrogen and oxygen react, they form water as indicated by the following equation.

2H2    +    O2      🠖      2H2O

If you had 1.52mol of hydrogen and 0.86mol of oxygen, which would be the limiting reactant and how many moles of water could be produced?