Answer:
1.1 x 10⁴ J
Explanation:
To calculate eth energy needed, you need to use the following equation:
Q = mcΔT
In this equation,
-----> Q = energy/heat (J)
-----> m = mass (g)
-----> c = specific heat (4.184 J/g°C)
-----> ΔT = change in temperature (°C)
You can plug the given values into the equation and solve.
Q = mcΔT
Q = (75.0 g)(4.184 J/g°C)(55.0 °C - 20.0 °C)
Q = (75.0 g)(4.184 J/g°C)(35.0)
Q = 11,000 J
Q = 1.1 x 10⁴ J
Sample cost = $15.796
<h3>Further explanation</h3>
Given
Mass = 2 g
Density = 0.718 g/ml
Cost = $5.67 per mL
Required
Cost
Solution
The density : the ratio of mass and volume
Can be formulated :
Density (ρ) = m : V
The volume of the liquid :
V = m : ρ
V = 2 g : 0.718 g/ml
V = 2.786 ml
Sample cost :
= 2.786 ml x $5.67/ml
= $15.796
Answer:
2.18×10⁴ kJ are liberated when you burn 0.554 kg of olive oil
Explanation:
The chart indicates that ΔH combustion for the olive oil is 39.31 kJ/g which means that, when you burn 1 g of olive oil, you have 39.31 kJ of heat.
In this case, the mass of olive is 0.554 kg. Let's convert the mass from kg to g → 0.554 kg . 1000 g / 1kg = 554 g
Now, the conversion factor:
554 g . 39.31 kJ / 1g = 2.18×10⁴ kJ
<span>After four half-lives 0.1 mole of the radioactive isotope would remain. If the amount of the isotope that remains after each half life is one half of previously existing amount. Half of 1.6 equals 0.8, half of 0.8 equals 0.4, half of 0.4 equals 0.2, and finally half of 0.2 equals 0.1 mole.</span>