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Mkey [24]
2 years ago
9

7. What produces more severe burns, boiling water or steam?​

Chemistry
1 answer:
Gwar [14]2 years ago
7 0

Answer:

boiling water

Explanation:

boiling water produces more severe burns

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In Period 2, as the elements are considered from left to
Elza [17]

Answer:

it will option B ,hope it helps

5 0
3 years ago
20 mL of 80°C water is mixed with 20 mL of 0°C water in a perfect calorimeter. What is the final temperature?
dedylja [7]
To calculate for the final temperature, we need to remember that the heat rejected should be equal to the absorbed by the other system. We calculate as follows:

Q1 = Q2
(mCΔT)1 = (mCΔT)2

We can cancel m assuming the two systems are equal in mass. Also, we cancel C since they are the same system. This leaves us,

 (ΔT)1 = (ΔT)2
(T - 80) = (0 - T)
T = 40°C
8 0
3 years ago
A box has a weight of 120 lbs and the bottom of the box is 12 in2 . What is the pressure the box exerts on the floor?
denis23 [38]
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7 0
3 years ago
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mixer [17]

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cell

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5 0
2 years ago
How much heat is released when 6.00 g of methane is combusted using the reaction below? CH4 + 2O2 ? CO2 + 2H2O ?Hrxn = -890. KJ
goblinko [34]

Answer : The amount of heat released is, -121.04 KJ

Solution : Given,

Enthalpy of reaction, \Delta H_{rxn} = -890 KJ

Mass of methane = 6 g

Molar mass of methane = 44 g/mole

First we have to calculate the moles of methane.

\text{Moles of methane}=\frac{\text{Mass of methane}}{\text{Molar mass of methane}}=\frac{6g}{44g/mole}=0.136moles

The given balanced reaction is,

CH_4+2O_2\rightarrow CO_2+2H_2O

From the balanced reaction we conclude that

1 mole of methane releases heat = -890 KJ

0.136 moles of methane releases heat = \frac{0.136moles}{1mole}\times -890KJ=-121.04KJ

Therefore, the amount of heat released is, -121.04 KJ

8 0
3 years ago
Read 2 more answers
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