The correct option is 14.0 g
Using the balanced thermochemical equation below, calculate the mass of hydrogen needed to release 642 kJ of heat....
Using the balanced equation shown below, calculate the mass of C3H8 that must react in order to release 2.850x106 kJ of heat. C3H8(g) +5O2 (8) → 3CO2(g) + 4H2O(g) ΔHrxn=-2219.9 kJ/mol
Question 14 5 pts The thermochemical equation for the reaction of nitrogen and hydrogen to form ammonia (NH3) is N2(g) + 3H2(g) -> 2NH3(g) AH = -92.22 kJ What is AH for reaction of 7.183 g of N2 in the above equation? Atomic weights of the elements encountered in this problem are as follows: H 1.00794 g/mol N 14.00674g/mol -47.29 kJ -85.41 kJ -23.65 kJ -68.19 kJ -12.35 kJ
This thermochemical expression is for the reaction of nitrogen(g) with hydrogen(g) to form ammonia(g). N2(g) + 3H2(g)2NH3(g) ΔrH = -92.2 kJ mol-1 Calculate the mass of N2(g) that must react to transfer 21.9 kJ to the surrounding in grams.
determine the amount of heat (in kj) given off when 4.53 * 10^4 g of ammonia is produced according to the equation below. assume that the reaction takes place under standard - state conditions at 25 celsius. N2(g) + 3H2(g) ---> 2NH3 ?H= -92.6 kJ/mol enter the answser in scientific notation
3. Use the thermochemical equations shown below to determine the enthalpy for the final reaction: N2(e) +202(g) → 2NOz (6) AH = ? Using (1) Nz (€) + 3H2(E) → 2NH3(g) AH = -92.2 kJ (2) 2NH, (g) + 4H20 (1) ► 2NO2 (g) + 7H2(g) AH = 1301.8 kJ (3) 2H20 (1) ► 2H2(g) + O2(g) AH = 571.6 kJ
The following thermochemical equation is for the reaction of iron(III) oxide(s) with hydrogen(g) to form iron(s) and water(g). Fe2O3(s) + 3H2(g)— 2Fe(s) + 3H2O(g) AH = 98.8 kJ When 62.3 grams of iron(III) oxide(s) react with excess hydrogen(g), kJ of energy are Hint: An amount of energy is expressed as a positive number. The sign of AH in the thermochemical equation indicates whether the energy is absorbed or evolved. An automobile engine provides 523 Joules of work to push the...
Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: N2(g) + 3H2(g) + 2NH3 (9) a What is the maximum mass of ammonia that can be produced from a mixture of 1.20 x 103 g N2 and 5.90 x 102 g H2? Mass = g
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3() – MgO(s) + CO2(g) AH = 117.3 kJ (a) Is heat absorbed or released in the reaction? released absorbed (b) What is AHrn for the reverse reaction? (c) What is AH when 3.10 mol of CO2 reacts with ercess Mgo? kJ (d) What is AH when 33.5 g of CO, reacts with excess 190? kJ
6. (2 points) Nitrogen gas and hydrogen gas react to produce ammonia and release heat as shown in the thermochemical equation below. a. If 25,356 J of heat were released in the reaction, what is the mass of ammonia that was produced? b. Is the reaction exothermic or endothermic? ) + 3 H2(g) → 2 NH3(g) Hrxn = -92.2 kJ
Consider the following balanced thermochemical equation for the decomposition of the mineral magnesite: MgCO3(s) - MgO(s) + CO2(g) AHrxn - 117.3 kJ (a) Is heat absorbed or released in the reaction? released o absorbed (b) What is AHfor the reverse reaction? (@) What is AH when 4.20 mol of CO, reacts with excess MgO? kJ (d) What is AH when 30.0 g of CO, reacts with excess MgO?