Answer:
66800 J
Explanation:
From the question given above, the following data were obtained:
Mass (m) = 200 g
Heat (Q) required =?
The heat required to melt the 200 g sample of water can be obtained as:
Mass (m) = 200 g
Latent heat of water (L) = 334 J/g
Heat (Q) required =?
Q = mL
Q = 200 × 334
Q = 66800 J
Thus, 66800 J of heat energy is required to melt the sample of water.
Answer:
1.35
Explanation Use the mole formla and multiply and them apply the sig fig rules and you will get the moles of water hope this helps god bless
Answer: 1.98 g
Explanation:
To calculate the moles :
The balanced given equation is:
According to stoichiometry :
4 moles of 
will produce = 2 moles of 
Thus 0.22 moles of will produce=
of
Mass of 
Thus 1.98 g of water is produced along with 5.0 L of at STP
The correct answer is option 3. A real gas behaves least like an ideal gas under the conditions of high temperature and low pressure. At this temperature and pressure, the molecules are close to each other and collisions or interactions are very likely to happen which is not an ideal gas.
Answer:
I <em>believe</em> it is Avogadro's number: 6.022 × 10²³
Explanation:
One mole of a substance is equal to 6.022 × 10²³ units of that substance
