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part 1: suppose that coal of density 1.5g/cm3 is pure carbon. the combustion of carbon is described by the question C(s)+ 02(g)- CO2 H= -394kJWhat is the value of heat when a lump of coal of size 7.3 cm x 6.8cm x 6.3cm is burned?part 2: what mass of water can be heated from 40C to 100C by burning this piece of coal? answer in units of g
If it takes 526 J of energy to warm 7.40 grams of water by 17 degrees Celsius, how much energy would be needed to warm 7.40 grams of water by 55 degrees Celsius?
A 275-g sample of nickel at 100.0C is placed in 100.0 mL of water at 22.0C. What is the final temperature of the water.
Description of Intermolecular forces, What parts of the calcium chloride are attracted to what parts of the water molecule when calcium chloride dissolves
A gaseous mixture of O2 and Kr has a density of 1.184 g/L at 385 torr and 300. K. What is the mole percent O2 in the mixture?
BNCT relies on the initial targeting of tumor cells by an appropriate chemical compound tagged with 10 5 B , which preferentially concentrates in tumor cells.
4.00 mL of 2.0E-3 M iron(III) nitrate solution is mixed with 5.00 mL of 2.0E-3 M potassium thiocyanate solution, 6.00 mL of 0.500 M nitric acid solution
if you burn 1.5 mol C3H8 according to the following reaction C3H8 +5O2 = 3CO2 + 4H2O how many grams of carbon dioxide are produced.
A solvent for an industrial process requires the use of phenol or benzene. Both are about the same in effectiveness for the process, and of course, gloves will be used when handling either solvent
Determine the mass of the steel bar if the final temperature of the system is twenty one degree Celsius?
In the first 12.0 of the reaction, 1.8×10-2 of is produced in a reaction vessel with a volume of 0.260 . What is the average rate of the reaction over this time interval.
Elements in the first short period are limited by the octect rule whereas those in the higher period can expand their valence shells. Describe what this means, account for this phenomenon and give an example of each.
Consider the reaction 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s). If 12.5 g of iron(III) oxide (rust) are produced from 8.74 g of iron, how much oxygen gas is needed for this reaction?
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