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salantis [7]
3 years ago
12

A scientific model must make a testable prediction. a scientific model must make a testable prediction.

Chemistry
1 answer:
Levart [38]3 years ago
8 0
It is true because Scientists will create models (simplified views of reality) to help them focus on the basic fundamental processes.
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Define physical change and give an example
Musya8 [376]
Physical isn't so chemical

6 0
3 years ago
Read 2 more answers
The enthalpy of fusion of solid n-butane is 4.66 kJ/mol. Calculate the energy required to melt 58.3 g of solid n-butane.
adelina 88 [10]

Answer : The energy required to melt 58.3 g of solid n-butane is, 4.66 kJ

Explanation :

First we have to calculate the moles of n-butane.

\text{Moles of n-butane}=\frac{\text{Mass of n-butane}}{\text{Molar mass of n-butane}}

Given:

Molar mass of n-butane = 58.12 g/mole

Mass of n-butane = 58.3 g

Now put all the given values in the above expression, we get:

\text{Moles of n-butane}=\frac{58.3g}{58.12g/mol}=1.00mol

Now we have to calculate the energy required.

Q=\frac{\Delta H}{n}

where,

Q = energy required

\Delta H = enthalpy of fusion of solid n-butane = 4.66 kJ/mol

n = moles = 1.00 mol

Now put all the given values in the above expression, we get:

Q=\frac{4.66kJ/mol}{1.00mol}=4.66kJ

Thus, the energy required to melt 58.3 g of solid n-butane is, 4.66 kJ

7 0
3 years ago
HURRY PLEASE
densk [106]

Answer:

C

Explanation:

on edg

7 0
3 years ago
**98 POINTS**
Andrei [34K]

OP already did it - CONGRATS!!

here are the steps 2 get the same ans:

(NH4)2 CO3 has 2x N, 8x H, 1x C and 3x O per molecule

so its molecular mass = 2x14 + 8x1 + 1x12 + 3x16

=28+8+12+48

=96g

of that 96g, 8x1=8g is due to Hydrogen

so by ratio n proportion, 1.00g will have 1x8/96 = 1/12g = 0.083g of H

3 0
3 years ago
NEED URGENT HELP WITH QUESTION ABOVE!!!!!!!!!!
My name is Ann [436]

Answer:

1.818x10²³ particles

Explanation:

Add the two atomic masses given to get 74.55 g.

Divide the number of grams given by the molar mass of KCl:

22.5g ÷ 74.55 = 0.302 mol

Multiply the moles by 6.022×10²³ particles

7 0
3 years ago
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