to determine the gas constant R, two students A and B perform an experiment based on the ideal gas equation given as Pv=RT. Both use the same gaseous sample having v=16.6m^3/mol and reported the approximate value of R as 8.3J/(K ∆ mol)
Answers
Answer:
A HAS BETTER FIT THAN B
SSE OF A IS 14
Step-by-step explanation:
Answer:
B has a better fit than A, hence correct
Step-by-step explanation:
Step : 1 Compared to BB, A fits better. A has an R2 of 0.643, while B has an R2 of 0.837.
Compared to A, B has a superior fit. Since R2 of A is less than R2 of B, the R2 of A is 0.643 and R2 of B is 0.837.
B is right since it fits better than A.
They don't fit the same since R2 doesn't match, thus the conclusion is erroneous.
SSE of A is 6.7, not 14. hence it's also false.
SSE of A is 6.7, not 11.4 hence it's also false.
SSE of A and B are not 14 it's also false.
Step : 2 PV=n RT is the state equation for a hypothetical ideal gas. The ideal gas law explains how the behaviour of an ideal gas sample relates to its pressure, temperature, volume, and molarity (P, T, V, and m) (n). The universal gas constant is denoted by the letter "R" in the equation PV=nRT.
Step : 3 When you are given three of a gas's four properties—pressure, volume, number of moles, and temperature—use this equation. The union of pressure and velocity is known as pressure-velocity. In other words, the dynamic seal interface's surface speed multiplies the system pressure.
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