Calculate the energy in Joules required to raise 80.0 grams of water (C=4.18 J/gC), 16.0 degrees

When 6.54 grams of Zn is placed in 500.0 mL of 1.00 M CuSO4(aq) in a coffee cup calorimeter, it reacts completely to displace copper. The temperature of the solution rises from 20.0˚C to 30.4˚C. Assume the coffee cup itself gains no heat and that the solution has the same density (1.00 g/mL) and specific heat (4.184 J/g˚C) as pure water. (a) How much heat does the solution gain during this reaction? (in J)

How much heat (in Joules) is gained by 157 grams of water thát is warmed from 25.0 °C to 74.0°C? The specific heat of water is 4.184 J g °C

Calculate the energy required (in units of kJ) to heat 12.00 g water from 22.00 oC to 115.0 oC? Specific heat capacity for liquid water is 4.184 J/(g·oC), the heat capacity for water vapor is 2.000 J/(g·oC).  The heat of vaporization for water in the gaseous state is 2260.0 J/g.

If 30.5 g of LiBr are dissolved 350.0 g of water at 20.0 °C in an insulated container, a temperature change is observed. The Δ H of solution of LiBr is -48.8 kJ/mol. Assuming that the specific heat of the solution is 4.184 J/(g C) and that no heat is gained or lost by the container, what will be the final temperature of the solution?

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First, a 5.500 g tablet of benzoic acid (C6H₂CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 19.00 °C to 45.03 °C over a time of 12.0 minutes. Next, 4.840 g of acetylene (C₂H₂) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 19.00 °C to 56.59 °C. Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: Is this reaction exothermic, endothermic, or neither? If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in the second experiment. Calculate the reaction enthalpy ΔΗ per mole of C₂H₂. rxn 2C₂H₂(g) + 50₂ (8) 4C0₂(g) + 2 H₂O (g) Be sure any of your answers that are calculated from measured data are…

A nickel at 30 °C is dropped into a glass of 15.0 g soda at 3.0 °C, if the heat capacity of the nickel is 4.40 J/°C, the heat capacity for the glass is 11.1 J/°C, and the soda has the same specific heat capacity as water (4.184 J/g°C), what is the final temperature of the mixture?

When a 45.0 g sample of an alloy at 100.0 °C is dropped into 55.0 g of water at 25.0 °C, the final temperature is 30.4 °C. What is the specific heat of the alloy? The specific heat of H2O(l) is 4.184 J·g–1·°C–1.            (A) 0.397 J·g–1·°C–1.           (B) 0.447 J·g–1·°C–1.           (C) 1.28 J·g–1·°C–1.           (D) 1.55 J·g–1·°C–1.

Humans are heterotrophs that consume food for energy. These foods comprise of sugars that are broken down by enzymic activity within the body for producing energy. This process, called cellular respiration, occurs according to the chemical equation: C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1 a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of theequilibrium constant (Kc) and predict the whether the products or reactants will befavoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are[CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reactionquotient (Qc). Compare the Kc and Qc values and predict the favoured direction of thereaction.d) Explain the effect on equilibrium ofi) Increasing temperatureii) Increasing…