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Wilburn Stoltenberg

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โˆ™ 2021-02-26 23:17:29
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A polynomial of degree zero is a constant term

The grouping method of factoring can still be used when only some of the terms share a common factor A True B False

The sum or difference of p and q is the of the x-term in the trinomial

A number a power of a variable or a product of the two is a monomial while a polynomial is the of monomials

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โˆ™ 2012-02-23 18:50:13

lol do it yoursel'

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Q: What is the viscosity of honey using the equation V equals 2 times deltaP times g times a squared divided by 9v?
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Theorem that states that an impulse produces a change in momentum?

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Can an exothermic reaction have positive enthalpy?

Typically, exothermic reactions have negative enthalpy, But this may not always necessarily be the case. To prove this we say that H=U+PV and U=Q+W (H=enthalpy, U=internal energy, P=pressure, V=volume, Q=heat, W=work). H=U+PV Substitute for U (see above) H=Q+W+PV Take the differential of dH: dH=dQ+dW+d(PV) Plug in for dW with dW=-P(deltaV)) (this is true for a ideal gas expanding against constant external pressure) dH=dQ-P(deltaV)+d(PV) Take the derivative of d(PV) using the chain rule dH=dQ-P(deltaV)+P(deltaV)+V(deltaP) Cancel like terms dH=dQ+V(deltaP) At constant pressure (which is what is normally observed in almost all naturally occurring environments the pressure is constant so the V(deltaP) term is 0 (change in volume is zero) and therefore dH=dQ. So in this case, if Q is negative so is enthalpy. However, if are at constant volume conditions (example: a bomb calormiter) where the pressure can change it may be possible to have a V(deltaP) term that is greater than the negative Q (indicating the reaction is exothermic while still giving you a positive enthalpy. Example: dQ=-1000J (Exothermic process) V=(5L) deltaP=2atm dH=dQ+V(deltaP) dH=-1000J+10L*atm=-1000J+1013.25J=13.25... (10Latm=1013.25J) dH is positive while the process is exothermic. I understand these conditions are extreme and unlikely, but they are being used to illustrate a point - mathematically, and potentially IRL, it is plausible to have an exothermic process with a positive change in enthalpy.

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