Answer:
Mass = 1.42 g
Explanation:
Given data:
Amount of heat absorbed = 4.56 j
Initial temperature = 29°C
Final temperature = 36°C
Mass of iron metal = ?
Specific heat capacity of iron = 0.46 j/g.°C
Solution:
Formula:
Q = m.c. ΔT
Q = amount of heat absorbed or released
m = mass of given substance
c = specific heat capacity of substance
ΔT = change in temperature
ΔT = T2 - T1
ΔT = 36°C - 29°C
ΔT = 7°C
Q = m.c. ΔT
m = Q / c. ΔT
m = 4.56 j / 0.46 j/g°C . 7°C
m = 4.56 j /3.22 j/g
m = 1.42 g
Answer:
838 torr
Step-by-step explanation:
To solve this problem, we can use the <em>Combined Gas Laws</em>:
p₁V₁/T₁ = p₂V₂/T₂ Multiply each side by T₁
p₁V₁ = p₂V₂ × T₁/T₂ Divide each side by V₁
p₁ = p₂ × V₂/V₁ × T₁/T₂
<em>Data:
</em>
p₁ = ?; V₁ = 2.42 L; T₁ = 27.0 °C
p₂ = 754 torr; V₂ = 2.37 L; T₂ = -8.8 °C
Calculations:
(a) Convert <em>temperatures to kelvins
</em>
T₁ = (27.0 + 273.15) K = 300.15 K
T₂ = (-8.8 + 273.15) K = 264.35 K
(b) Calculate the<em> pressure
</em>
p₁ = 754 torr × (2.37 L/2.42) × (300.15/264.35)
p₁ = 754 torr × 0.979 × 1.135
p₁ = 838 torr
Answer:
So if this is about chemical equations. You have 3 steps.
Step 1.- Count each type of atom in reactants and products.
Step 2.- Place coefficients, as needed, in front of the symbols or formulas to increase the number of atoms or molecules of the substances.
Step 3.-Repeat steps 1 and 2 until the equation is balanced.
Explanation:
Answer: I believe the answer is A, heat moves from warmer objects to cooler objects. I know for sure it isn’t C or D though so A