Answer:
1.57 x 10⁷m
Explanation:
Given quantity is;
1.57 x 10¹⁴nm
Now;
1 nm = 10⁻⁹
So, let us convert this given quantity;
1 nm = 10⁻⁹
1.57 x 10¹⁴nm will give 1.57 x 10¹⁴ x 10⁻⁹ = 1.57 x 10⁷m
The correct answer is c.
answer b is incorrect <span />
Answer:
172.23L
Explanation:
Data obtained from the question include:
V1 (initial volume) = 200 L
P1 (initial pressure) = 0.94 atm
T1 (initial temperature) = 25°C = 25 + 273 = 298K
P2 (final pressure) = 1atm
T2 (final temperature) = 0°C = 0 + 273 = 273K
V2 (final volume) =?
Using the general gas equation P1V1/T1 = P2V2/T2, the final volume of the container can be obtain as follow:
P1V1/T1 = P2V2/T2
0.94 x 200/298 = 1 x V2/273
Cross multiply to express in linear form as shown below:
298 x V2 = 0.94 x 200 x 273
Divide both side by 298
V2 = (0.94 x 200 x 273)/298
V2 = 172.23L
The new volume of the container is 172.23L
The specific heat capacity of the metal is determined as 0.76 J/g⁰C.
<h3>Mass of the water</h3>
mass = density x volume
mass = 342 ml x 1 g/ml = 342 g
<h3>Specific heat capacity of the metal</h3>
Apply the law of conservation of energy;
Heat lost by the metal = Heat gained by the calorimeter + heat gained by water
(93.4)(85 - 29.3)c = (8.29)(29.3) + (342)(4.186)(29.3 - 26.7)
5,202.38c = 3,965.088
c = 3,965.088/5,202.38
c = 0.76 J/g⁰C
Thus, the specific heat capacity of the metal is determined as 0.76 J/g⁰C.
The complete question is below;
93.4 g of a metal is heated to 85.0 C in a hot water bath, then dropped into a calorimeter containing 342 ml of water (d 1.00 g/mL) at 26.7 . The equilibrium temperature was found to be 29.3 C. Calculate the specific heat of the metal with proper units. (C.cal 8.29 J/c)
Learn more about specific heat capacity here: brainly.com/question/16559442
#SPJ1