Answer:
Explanation:
This is a direct application of the equation for ideal gases.
Where:
- P = pressure = 1.25 atm
- V = volume = 25.2 liter
- R = Universal constant of gases = 0.08206 atm-liter/K-mol
- T = absolute temperature = 25.0ºC = 25 + 273.15 K = 298.15 K
- n = number of moles
Solving for n:
Substituting:
Answer:
We can use heat = mcΔT to determine the amount of heat, but first we need to determine ΔT. Because the final temperature of the water is 55°C and the initial temperature is 20.0°C, ΔT is as follows:
ΔT = Tfinal − Tinitial = 55.0°C − 20.0°C = 35.0°C
given the specific heat of water as 1 cal/g·°C. Substitute the known values into heat = mcΔT and solve for amount of heat:
= heat=(75.0 g)(1 cal/ g· °C )(35.0°C) =
= 75x1x35=2625 cal
Explanation:
The scientific notation:
where
and k is integer.
We have the example:
You can write the numbers in a "normal" form:
Make the sum:
And next write it in the scientific notation:
<h3>Other method:</h3>
You can add numbers in scientific notation if the power of tens in both number is the same.
Therefore you must convert the first number:
Now, you can make the sum:
Explanation:
Thus, those metals which remain unaffected by moisture, oxygen and carbon dioxide of the air can occur native or free. In other words, the unreactive metals occur in nature in free state because of their low reactivity towards chemical reagents. ... Metals usually occur in combination with nonmetallic elements.
<span>2 C2H6(g) + 5 O2(g) --------> 4 CO(g) + 6 H2O(g)
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