Answer:
partial pressure of gas D Pd = 15.5 kPa
Explanation:
As per the Dalton's law of partial pressure, in a mixture, pressure exerted by each gas when summed gives the total partial pressure exerted by mixture.
P(Total) = P1+P2+P3.....
Given P(Total) = 35.7 kPa
Partial pressure of gas A Pa = 7.8 kPa
Partial pressure of gas B Pb = 3.7 kPa
Partial pressure of gas C Pc = 8.7 kPa
There, Partial pressure of gas D Pd = P(Total) -(Pa+Pb+Pc)
Pd = 35.7-(7.8+3.7+8.7) = 35.7-20.2 kPa = 15.5 kPa
Therefore, partial pressure of gas D Pd = 15.5 kPa
Answer:
carbon dioxide
Explanation:
Carbon burns in oxygen to form carbon dioxide. Since hydrocarbon fuels only contain two elements, we always obtain the same two products when they burn. In the equation below methane (CH 4) is being burned. The oxygen will combine with the carbon and the hydrogen in the methane molecule to produce carbon dioxide (CO 2) and water (H 2O).
Carbon, as graphite, burns to form gaseous carbon (IV) oxide (carbon dioxide), CO2. ... When the air or oxygen supply is restricted, incomplete combustion to carbon monoxide, CO, occurs. 2C(s) + O2(g) → 2CO(g) This reaction is important. When one mole of carbon is exposed to some energy in the presence of one mole of oxygen gas, one mole of carbon dioxide gas is produced. This reaction is a combustion reaction.
A. ca is the answer because its short for carbon
The question here is solved using basic chemistry. CaCl2(aq) is an ionic compound which will have the releasing of 2 Cl⁻ ions ions in water for every molecule of CaCl2 that dissolves.
CaCl2(s) --> Ca+(aq) + 2 Cl⁻(aq)
[Cl⁻] = 0.65 mol CaCl2/1L × 2 mol Cl⁻ / 1 mol CaCl2 = 1.3 M
The answer to this question is [Cl⁻] = 1.3 M
The Law of Conservation of Mass states that matter can neither be created nor destroyed in a chemical reaction.
