The empirical formula, <span>C<span>H2</span></span>, has a relative molecular mass of
<span>1×<span>(12.01)</span>+2×<span>(1.01)</span>=14.04</span>
This means that the empirical formula must be multiplied by a factor to bring up its molecular weight to 70. This factor can be calculated as the ratio of the relative masses of the molecular and empirical formulas
<span><span>7014.04</span>=4.98≈5</span>
Remember that subscripts in molecular formulas must be in whole numbers, hence the rounding-off. Finally, the molecular formula is
<span><span>C<span>1×5</span></span><span>H<span>2×5</span></span>=<span>C5</span><span>H<span>10</span></span></span>
Answer:True.
As you increase the wavelength the frequency decreases.
Explanation:
The wavelength of a wave is the distance(in meters) between the two consecutive crest and trough of a wave. The S.I unit of the wavelength is meter.
The frequency of a wave is the number of complete wave cycle passing a particular point per second. The S.I unit of the frequency is Hertz.
Wave's frequency and wavelength are related to each other as
Frequency = 1 / Wavelength
As the Frequency is inversely proportional to the wavelength of a wave so as the frequency will increase the wavelength of the wave will decrease and vise-versa.
So, its true that As we increase the wavelength the frequency decreases.
You didn't put the reactions
Answer:
Before we go through this I ask you carefully read every thing I've listed out or it's not going to make sense for you.
The equation:
CO2 and O2 aren't reacting with each other. One is a product and the other is a reactant. You're probably asking for how much CO2 will be formed with 17 moles of O2. It's pretty simple.
First you have to find the mole to mole ratio of O2 to CO2 (look at their coefficients/numbers right in front of their names), the ratio is 9 : 6, so for every 9 of oxygen gas (O2), 6 of carbon dioxide (CO2) is made. We have 17 moles of oxygen so if we divide it by 9 (mole ratio of oxygen gas) and multiply it by 6, we will get the amount of CO2 produced.
<u>(17/9) x 6 ≈ 11.3 moles of CO2 are made. </u>
In the case that you actually meant to say C3H7OH (Propanol) reacting with oxygen, I'll write that down here too:
The mole to mole ratio of Propanol to Oxygen gas is 2 : 9 (look at the coefficients) so we divide 17 moles of oxygen by 9 and then multiply it by 2, which will give us the amount of Propanol needed.
<u>(17/9) x 2 = 3.78 moles of Propanol is required to react with oxygen.</u>
Answer:
Alcohol ( ethanol ) C2H6O.
Alka Seltzer* ( sodium bicarbonate )
Antifreeze ( ethylene glycol ) ...
Antiperspirant (aluminum chlorohydrate) ...
Aspirin* ( acetylsalicylic acid ) ...
Baking powder ( sodium bicarbonate¶ ) ...
Battery acid ( sulphuric acid ) ...
Bleach, laundry ( sodium hypochlorite )
Explanation: