1. The problem statement, all variables and given/known data A pop-up turkey thermometer has 1.0 mL of air trapped beneath the red plastic indicator. When the thermometer was assembled, the temperature was 10 *C, and atmosphereic pressure was 750 mmHg. If the pressure required to break the seal and pop up the syringe is 932 mm Hg, at what temperature in *F will the turkey be done? 2. Relevant equations PV=nrT *C x 9/5 + 32 = *F *C + 273 = *K P_1V_1=P_2V_2 1 atm = 760 mmHg P_1V_1/n_1T_1=P_2V_2/n_2T_2 (I'm not sure if I need this one or not) 3. The attempt at a solution First, I started computing my starting variables. P_1 = 750/760 = .987 atm V_1= .001 L T_1= 283 *K n_1 = ? P_2= 932/760 = 1.23 atm V_2 = ? T_2 = ? n_2 = ? To continue, I need to find n. So I used the Ideal Gas Law (no excessive pressures). PV=nRT PV/RT=n (.987 atm)(.001 L)/(.0821 Lxatm/molxK)(283 *K) = 4.25 x 10^-5 mol air I assign this value to both n_1 and n_2, because the mols of air shouldn't change. When writing the combined gas law, I still need to find V_2 to find T_2. So I use Charle's Law. P_1V_1/P_2 = V_2 (.987 atm)(.001 L)/(1.23 atm) = 8.02 x 10^-4 This is where I'm uncertain. I rearrange the combined gas law to look like this: P_1V_1n_2/P_2V_2n_1T_1 = T_2 Plug in my numbers, I get 3.54 x 10^-3 *K. That's rediculous, considering the context of the problem. So I try to use the Ideal Gas Law, but only on the second state of gas PV=nRT manipulated to PV/nR=T (1.23 atm)(.001 L)/(4.248 x 10^-5 mol)(.0821 L x atm/mol x K) = 353 *K. A much more reasonable answer. I convert to C, and get 80 *C. I think I've got it. Convert to *F, and I get 176 *F. But the computer says I'm wrong. Where did I mess up? Help please?