Thalia needs to factor in the sphere's size, its mass, the necessary permits, and the overall expenses for its fabrication.
Answer:
The temperature increase of the calorimeter, which is missing in the problem, is necessary for the calculation.
Explanation:
Since the temperature rise (X) is unspecified, we'll express the calculation in terms of X, and demonstrate with an example value.
1) Calorimeter details:
- Temperature increase: X °C
- Heat capacity ratio: 4.87 J / 5.5 °C (given)
- Energy absorbed by calorimeter at X °C rise:
(4.87 J / 5.5 °C) × X
2) Reaction data:
- Heat released: 362 kJ per mole of reactant
- Number of moles consumed: n
- Total energy from reaction:
362 kJ/mol × 1000 J/kJ × n = 362,000 n J
3) Using energy conservation, assuming no heat loss to surroundings, the energy from the reaction equals the energy absorbed by the calorimeter:
- 362,000 n = (4.87 J / 5.5 °C) × X
- n = [(4.87 / 5.5) × X] / 362,000
n = 0.000002446 × X
This means for each degree Celsius rise in calorimeter temperature, 0.000002446 moles of reactant were consumed.
Example:
If the calorimeter temperature increases by 100 °C, then:
- n = 0.000002446 × 100 = 0.0002446 mol
The responses to the question are: a. True b. True c. True d. False Explanation: The relevant relationship is given as the gas constant R, with T being the temperature in Kelvin, and m being the molecular mass, while represents the root mean square speed. Evaluating the kinetic energy equations lead us to the conclusion that: a. Increasing the temperature of a gas sample raises root-mean-square speed, hence true. b. At the same temperature, gases share equal average kinetic energy; thus true. c. When gas temperatures rise, the count of particles with average kinetic energy increases, affirming true. d. However, equal temperature does not ensure identical root-mean-square speeds due to varying molecular masses in different gases, which leads to this statement being false.
The thickness of the metal sheet measures 1.93 mm.
Answer:
334 J/g
Explanation:
The relevant data provided in the question are as follows:
Mass (m) = 1 g
Specific heat of Fusion (Hf) = 334 J/g
Heat (Q) =?
By applying the formula Q = m·Hf, we can calculate the heat released:
Q = m·Hf
Q = 1 x 334
Q = 334 J
Thus, the total heat released amounts to 334 J.
